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CHEM 231 > Quiz 1 - Solids > Flashcards

Quiz 1 - Solids Flashcards

(55 cards)

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1
Q

Define crystal structure

A

3D arrangement of atoms

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2
Q

Solids can be one of two types

A

crystalline or amorphous

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3
Q

Define crystal lattice

A

pattern formed by repeating structural elements

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4
Q

Define unit cell

A

smallest repeat unit of a crystal structure that reproduces the crystal in 3D

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5
Q

List the 7 crystal systems

A

Cubic, tetragonal, orthorhombic, monoclinic, triclinic, trigonal, hexagonal

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6
Q

What is the relationship between lattice parameters for orthorhombic?

A

a does not equal b does not equal c, A=B=Y=90

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7
Q

What is the relationship between lattice parameters for rhombohedral (trigonal)

A

a=b=c, A=B=Ydoesnt= 90

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8
Q

What is the relationship between lattice parameters for tetragonal?

A

a=bdoesnt=c, A=B=Y=90

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9
Q

What is the relationship between lattice parameters for hexagonal?

A

a=bdoesnt=c, A=B=90, Y=120

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10
Q

What is the relationship between lattice parameters for cubic?

A

a=b=c, A=B=Y=90

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11
Q

ABA = what? ABC = what?

A

ABA = hexagonal close packed, ABC = cubic close packed

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12
Q

CCP and HCP have the same ___

A

packing density (74%) and Cn = 12

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13
Q

How many holes in CCP and HCP? How big are they?

A

N octahedral holes, 2N tetrahedral holes
Octahedral hole is 0.41r, tetrahedral is 0.23r

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14
Q

What is an example of non close packing?

A

BCC body centered cubic

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15
Q

What is the packing density of BCC?

A

68%

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16
Q

Are ionic structures truly close packed CCP or HCP?

A

no, eutectic, anions dont actually touch due to electrostatic replusion

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17
Q

The radius of the cation must be ____ than the hole it sits in?

A

greater

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18
Q

What do the different CNs mean in a unit cell?

A

structure but not shape of cell
CN = 8 = cubic
CN = 6 = octahedral
CN = 4 = tetrahedral
CN = 3 = trigonal planar
CN = 2 = linear

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19
Q

Give an example of an AB structure with CN = 8 (cubic)

A

CsCl - cubic

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20
Q

Give an (2) example of an AB structure with CN = 6 (octahedral)

A

NaCl - cubic
NiAs - hexagonal

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21
Q

Give an (2) example of an AB structure with CN = 4 (tetrahedral)

A

ZnS (zinc blende) - cubic
ZnS (Wurtzite) - hexagonal

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22
Q

Give an example of an AB2 structure with CN = 8-4, 6-3, 4-2,

A

CaF2 (fluorite) - cubic
TiO2 (Rutile) - tetragonal
SiO2 (Cristabolite) cubic

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23
Q

Give an example of an A2B structure

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A

Anti fluorite K2O

24
Q

If the radius ratio is 0.225-0.414 then…

Study These Flashcards
A

AB - ZnS (ccp and hcp)

25
If the radius ratio is 0.414-0.732 then....
AB - NaCl (ccp), NiAs (hcp) AB2 - TiO2
26
If the radius ratio is 0.732-1 then...
AB - CsCl AB2 - CaF2
27
What is the shottky defect?
missing atoms, charge has to be neutral
28
What is the Frenkel defect?
Displacement into interstitial sites
29
What is anti site disorder?
+/- atoms are swapped in one spot
30
What is an extrinsic defect?
If an atom of less or more charge is inserted into a structure, defects in sites having opposite charges will occur to balance
31
How do you determine the set of quantum numbers for a given element?
n= energy (shell) 1,2,3,4 l = s,p,f,d 0,1,2,3 (n-1) ml = l to -l
32
What is a node?
part in the function where the probability of finding an electron drops to 0
33
What are the exceptions for electron configurations?
Cr = [Ar] 4s1 3d5 Cu = [Ar] 4s1 3d10 (Same for 4d analogues - Mo and Ag)
34
How do you calculate effective nuclear charge in this course?
Zeff = #protons - #core electrons (not valence)
35
VESPER - 2 things
EPG = Linear - 0 LEP = Linear
36
VESPER - 3 things
EPG = Trigonal Planar - 0 LEP = Trigonal Planar - 1 LEP = Bent
37
VESPER 4 things
EPG = Tetrahedral - 0 LEP = Tetrahedral - 1 LEP = Trigonal Pyramidal - 2 LEP = Bent
38
VESPER 5 things
EPG = Trigonal Bipyramidal - 0 LEP = Trigonal Bipyramidal - 1 LEP = See Saw - 2 LEP = T shaped - 3 LEP = Linear
39
VESPER 6 things
EPG = Octahedral - 0 LEP = Octahedral - 1 LEP = Square pyramidal - 2 LEP = Square planar
40
Define the Pauli Exclusion principle
No two electrons in the same atom can have the same 4 QNs
41
Define Hunds rule
Degenerate orbitals are occupied separately by electrons with parallel spins
42
Ionization energy __ left to right and __ down
increases, decreases
43
Electronegativity ___ left to right
increases
44
Define constructive and destructive interference
Constructive - amplitude increases - more likely to find an electron here - bonding orbitals
45
Paramagnetic vs Dimagnetic?
Para = spins parallel (unpaired) - attracted to mag field Dia = spins paired - repelled from mag field
46
E neg differences?
0 - covalent 0.1-0.4 - NP covalent 0.5-1.7 - P covalent Greater than 1.7 = Ionic
47
The more e neg atom contributes more to the ___ orbital
bonding (opposite applies)
48
greater bond order = ___ bond strength = ___ bond length
greater, shorter (cuz pulling closer)
49
What is the difference between the MO energy diagrams between the diagram for Li - N and O - F?
Li - N is (bottom up) sigma sigma pi sigma pi sigma O - F is sigma sigma sigma pi pi sigma 2P is 2 down from top - 2S goes to 1,2,4 - 2P goes to 2,3,4,5,6 (Li - N) - 2S goes to 1,2 - 2P goes to 3,4,5,6 (O - F)
50
rule for transition metal ionizations with electron configurations?
if its a plus charge - remove from the 4s before the 3d
51
why are lewis diagrams bad?
no prediction of 3D structure or contributuion of resonance
52
Why is VSEPR bad?
works bad with heavy elements - must hybridize
53
Why is VB bad?
need lewis structure first - describes bonding but not energies
54
When is MO theory bad?
great predictor of energies but not good for determining structure
55
for heteronuclear diatomics we do not use?
EX) IBr - we do not use g and u

CHEM 231 (3 decks)

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